Molar Mass of Aluminum Iodide (AlI3)
Molar Mass of Aluminum Iodide is commonly used in ionic-equation practice and concentration calculations for salt solutions. Molar Mass of AlI₃ is 407.69 g/mol, based on 2 element types, with I contributing the largest share.
For fast checks, use the molar mass calculator, verify element values in the periodic table, or explore more molar mass page.
Molar Mass of Aluminum Iodide is:
407.69 g/mol
Molar Mass of AlI₃ equals 407.69 g/mol, so 407.69 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Aluminum (Al) | 1 | 26.98 | 1 x 26.98 | 26.98 g/mol |
| Iodine (I) | 3 | 126.90 | 3 x 126.90 | 380.71 g/mol |
Final molar mass 26.980 + 380.710 | 407.69 g/mol | |||
Computing Molar Mass of Aluminum Iodide Step by Step
Molar Mass of Aluminum Iodide: Step-by-Step Calculation
1. Identify Element Counts
Read AlI3 and list how many atoms of each element are present:
- 1 atom of Aluminum (Al)
- 3 atoms of Iodine (I)
2. Determine Atomic Masses
Look up each element mass from the periodic table:
- Aluminum (Al) ~= 26.982 g/mol
- Iodine (I) ~= 126.904 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Aluminum (Al): 1 x 26.982 = 26.980 g/mol
- Iodine (I): 3 x 126.904 = 380.710 g/mol
4. Sum Total Molar Mass
Add all contributions to get the final molar mass in g/mol.
Molar Mass = (1 x 26.982 + 3 x 126.904)
Molar Mass = 26.980 + 380.710
Molar Mass = 407.690 g/mol
Final rounded value shown on this page: 407.69 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Aluminum (Al) | 1 | 26.982 | 1 x 26.982 | = 26.980 |
| Iodine (I) | 3 | 126.904 | 3 x 126.904 | = 380.710 |
Final molar mass 26.980 + 380.710 | = 407.690 | |||
When you move to another formula, molar mass guide gives you the same step-by-step method for quick revision.
Easy Way to Remember
Easy way to remember Molar Mass of Aluminum Iodide
- Molar Mass of Aluminum Iodide: count atoms, multiply masses, and add totals.
- Write each element in a table so you do not miss subscripts.
- Keep 2-3 decimals during steps, then round only at the end.
Sample Reactions
| Type | Reaction |
|---|---|
| Double displacement | AgNO₃ + NaCl → AgCl + NaNO₃ |
| Acid-salt reaction | Na₂CO₃ + ₂HCl → ₂NaCl + H₂O + CO₂ |
Do You Know?
– Aluminum Iodide contains 2 element types: Al, I.
– I contributes the largest share of this compound's total molar mass.
– In AlI₃, I appears with the highest atom count.
– Its molar mass is 407.69 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Aluminum Iodide is double displacement (AgNO₃ + NaCl → AgCl + NaNO₃).
Why This Compound Matters
Aluminum Iodide appears in ionic-reaction practice and precipitation examples in school chemistry.
Its molar mass helps students move quickly between grams, moles, and concentration problems.
Similar calculations can be compared with Sodium Iodide (NaI) and Potassium Iodide (KI).
Where This Is Used
- Competitive exams and school chemistry tests.
- Lab work when preparing measured solutions.
- Real-world manufacturing and quality checks.
Common Mistakes When Calculating This
- Skipping subscripts in AlI₃ and miscounting atoms.
- Rounding atomic masses too early before finishing all multiplication steps.
- Mixing up I element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Aluminum Iodide.
Quick Revision
Formula: AlI3
Molar Mass: 407.69 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
AlI3 contains Aluminum (Al) (1), Iodine (I) (3). Add each element contribution to get total molar mass.
FAQ
What is the molar mass of AlI3?
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Where is AlI3 molar mass used?
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Does rounding affect my final AlI3 answer?
Conclusion
Molar Mass of Aluminum Iodide and Molar Mass of AlI₃ are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.